Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 22, Problem 22.36E
Interpretation Introduction
Interpretation:
The planes which have the atoms closest together in a cubic crystal are to be stated.
Concept introduction:
A unit cell of the crystal is the three-dimensional arrangement of the atoms present in the crystal. The unit cell is the smallest and simplest unit of the crystal which on repetition forms an entire crystal. Unit cell can be a cubic unit cell or hexagonal unit cell. The classification of a unit cell depends on the lattice site occupied by the atoms.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
c) Draw the 10 point coordinate in a cubic unit cell.
Determine the Miller indices for the directions in
the cubic unit cell
A
В
Directions in a cubic unit cell
-IN
Elemental silver reflects X-rays of wavelength 154.18 pm at angles of 19.076°, 22.171°, and 32.256°. However, there are no other reflections at angles of less than 33°. Assuming a cubic unit cell, determine its type and dimension. Calculate the mass density of silver. Hint: Calculate the expected reflections from different types of cubic unit cell and compare those with the data given.
Chapter 22 Solutions
Physical Chemistry
Ch. 22 - Using the explanation of unbalanced forces as the...Ch. 22 - Show that the right side of equation 22.1 has...Ch. 22 - The text claims that surface tension varies with...Ch. 22 - Prob. 22.4ECh. 22 - Prob. 22.5ECh. 22 - Prob. 22.6ECh. 22 - Prob. 22.7ECh. 22 - Equation 22.6 defines surface tension in terms of...Ch. 22 - Prob. 22.9ECh. 22 - Prob. 22.10E
Ch. 22 - Prob. 22.11ECh. 22 - Prob. 22.12ECh. 22 - Prob. 22.13ECh. 22 - Prob. 22.14ECh. 22 - Prob. 22.15ECh. 22 - Prob. 22.16ECh. 22 - Prob. 22.17ECh. 22 - Prob. 22.18ECh. 22 - Prob. 22.19ECh. 22 - Determine the pressure difference on a droplet of...Ch. 22 - Prob. 22.21ECh. 22 - Prob. 22.22ECh. 22 - Prob. 22.23ECh. 22 - Prob. 22.24ECh. 22 - Prob. 22.25ECh. 22 - Prob. 22.26ECh. 22 - Prob. 22.27ECh. 22 - The Young-Dupr equation, equation 22.16, is...Ch. 22 - Why are capillary rises and depressions not seen...Ch. 22 - Prob. 22.30ECh. 22 - Prob. 22.31ECh. 22 - Prob. 22.32ECh. 22 - Prob. 22.33ECh. 22 - Prob. 22.34ECh. 22 - Prob. 22.35ECh. 22 - Prob. 22.36ECh. 22 - Prob. 22.37ECh. 22 - Prob. 22.38ECh. 22 - A china cup breaks when the ionic or covalent...Ch. 22 - Satellites in space often suffer from vacuum...Ch. 22 - Prob. 22.41ECh. 22 - Prob. 22.42ECh. 22 - Prob. 22.43ECh. 22 - Are the following processes examples of...Ch. 22 - Prob. 22.45ECh. 22 - Early attempts to coat metals with Teflon, poly...Ch. 22 - Prob. 22.47ECh. 22 - Prob. 22.48ECh. 22 - Prob. 22.49E
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Describe the unit cell of lithium (see Figure).arrow_forwardHow many different unit cells can a crystal have if the unit cell a has all 90 angles between its crystal axes; b has all of its unit cell dimensions the same length; c has at least one 90 angle between axes; d has no perpendicular axes or equivalent unit cell dimensions?arrow_forwardThe test tubes shown here contain equal amounts of the specified motor oils. Identical metal spheres were dropped at the same time into each of the tubes, and a brief moment later, the spheres had fallen to the heights indicated in the illustration. Rank the motor oils in order of increasing viscosity, and explain your reasoning:arrow_forward
- The coordination number of uniformly sized spheres in a cubic closest-packing (FCC) array is 12. Give the coordination number of each atom in (a) a simple cubic lattice. (b) a body-centered cubic lattice.arrow_forwardHelp questions 1&2arrow_forwardWhat does the simple cubic unit cell consist of?arrow_forward
- The results of a X-Ray Diffraction experiment using X-Rays with A=1.54Å show that diffracted peaks occur at the following 20 angles: Peak 20 Peak 20 46.0 4 102.8 67.1 5 121.8 3 85.2 6 146.3 Determine the crystal structure, the indices of the plane producing each peak and the lattice parameter of the material. 2d sint=nd Recall that: for cubic structures. heearrow_forwardEquivalent lattice points within the unit cell of a Bravais lattice have identical surroundings. What points within a body-centered cubic unit cell are equivalent to the point (1/2, 0, 1/2) ?arrow_forwardIt is not possible to pack spheres together without leaving some void spaces between the spheres. Packing efficiency is thefraction of space in a crystal that is actually occupied by atoms. Determine the packing efficiency of a face-centered cubic metal.arrow_forward
- what are antiferromagnetic and ferromagnetic solids?arrow_forwardGive some examples of Covalent-network solids?arrow_forward1. Simple Cubic Unit Cell (b) Fig 5. Simple Cubic (SC) Unit Cell. (a) Ball-and-Stick Model (b) Space-filled Model (c) Stacking (a) a. Each corner atom of the unit cell would be shared by how many unit cells? Answer: b. Assuming the atoms as perfect spheres, how much of a corner atom is used by just a single unit cell? Answer: c. If there are atoms at the eight corners of a simple cubic cell and each atom is shared by eight unit cells, how many total atoms are there per simple cubic unit cell? Answer:arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning